Final Exam Review Questions and Answers All Units
A
10) At constant pressure, which graph shows the correct relationship between the volume of a gas (V) and its absolute temperature (T)? A) A B) B C) C D) D
B
10) How many joules of heat energy are needed to completely melt 25.0 grams of ice to water at 0*C? A) 56,500 J B) 8,350 J C) 334 J D) 105 J
A
10) The diagram below shows the data collected during the heating of a 5.0-gram sample of a hydrated salt. What is the percent water in the original sample? A) 40.% B) 30.% C) 60.% D) 82.%
A
10) What is the molality of a solution of KNO3 (formula mass = 101.1) that contains 202.2 grams of solute dissolved in 500 grams of water? A) 4 m B) 0.2 m C) 2 m D) 0.4 m
A
10) When the equation __Al + __O2 -> __Al2O3 is correctly balanced using smallest whole numbers, the sum of the coefficients will be A) 9 B) 12 C) 7 D) 3
C
11) A 25.0 gram sample of a substance absorbs 3,750 joules of heat energy to melt completely at its melting temperature. What is the heat of fusion of the substance? A) 8,350 J/g B) 334 J/g C) 150. J/g D) 2,260 J/g
C
11) A sample of oxygen gas has a volume of 150. milliliters at 300 K. If the pressure of the sample is held constant and the temperature is raised to 600 K, the new volume of the sample will be A) 75.0 mL B) 150. mL C) 300. mL D) 600 mL
B
11) Given the equation: __FeCl2 + __Na2CO3 -> __FeCO3 + __NaCl When the equation is correctly balanced using the smallest whole numbers, the coefficient of NaCl is A) 6 B) 2 C) 3 D) 4
C
11) How many moles of KCl are contained in 2,000 grams of a 0.2 molal solution? A) 30 B) 15 C) 0.4 D) 0.2
C
11) What is the empirical formula of the compound whose molecular formula is P4O10? A) P8O20 B) PO2 C) P2O5 D) PO
A
12) A 16.0-gram sample of CH4(g) is at 0*C and 1 atmosphere. The volume of the gas sample in liters at 27*C and 1 atmosphere is equal to A) 22.4 x 300/273 B) 16.0 x 1/27 C) 16.0 x 27/1 D) 22.4 x 273/300
A
12) A compound with an empirical formula of CH2 has a molecular mass of 70. What is the molecular formula? A) C5H10 B) CH2 C) C2H4 D) C4H8
B
12) Given the reaction: 2C2H6(g) + 7O2(g) -> 4CO2(g) + 6H2O(g) At STP, what is the total volume of CO2(g) formed when 6.0 liters of C2H6(g) are completely oxidized? A) 6.0 L B) 12 L C) 24 L D) 4.0 L
B
12) What conditions of pressure and temperature exist when ice melts at its normal melting point? A) 1 atm and 0 K B) 1 atm and 0*C C) 760 atm and 273 K D) 760 atm and 0*C
C
12) What is the mass of NaCl in 50 grams of a 10% solution? A) 0.5 g B) 0.2 g C) 5 g D) 10 g
B
12) When the equation NH3 + O2 -> HNO3 + H2O is completely balanced using smallest whole numbers, the coefficient of O2 would be A) 1 B) 2 C) 3 D) 4
C
13) A compound consists of 46.7% nitrogen and 53.3% oxygen by mass. What is its empirical formula? A) N2O B) N2O3 C) NO D) NO2
B
13) A gas sample is at 10.0*C. If pressure remains constant, the volume will increase when the temperature is changed to A) 263 K B) 293 K C) 283 K D) 273 K
A
13) What is the mass of KCl in 250. grams of a 5.0% solution? A) 12.5 g B) 1.25 g C) 5.0 g D) 2.0 g
C
13) Which equation best describes the reaction shown in the diagram? A) 2A + 6B -> A2B6 B) 3A + B -> 2AB C) A2 + 3B2 -> 2AB3 D) 3A2 + B2 -> 2A3B
C
13) Which phase change represents deposition? A) liquid ‚ gas B) solid ‚ liquid C) gas ‚ solid D) gas ‚ liquid
D
14) How many kilojoules of heat are absorbed when 70.00 grams of water is completely vaporized at its boiling point? A) 158,200 B) 2,260 C) 2.260 D) 158.2
B
14) The volume of a 1.00-mole sample of an ideal gas will decrease when the A) pressure decreases and the temperature decreases B) pressure increases and the temperature decreases C) pressure increases and the temperature increases D) pressure decreases and the temperature increases
D
14) What general type of reaction is illustrated in the diagram? A) decomposition B) double replacement C) single replacement D) synthesis
C
14) What is the empirical formula of a compound that contains 92.3% carbon and 7.7% hydrogen by mass? A) CH2 B) CH3 C) CH D) CH4
D
14) Which solution has the highest boiling point? A) 1 mole of NaNO3 in 1000 g of water B) 1 mole of NaNO3 in 750 g of water C) 1 mole of NaNO3 in 500 g of water D) 1 mole of NaNO3 in 250 g of water
D
15) A 16.0-gram sample of a compound containing only copper and sulfur is decomposed to produce 12.8 grams of copper and 3.2 grams of sulfur. What is the empirical formula of the compound? A) Cu2S3 B) CuS2 C) CuS D) Cu2S
D
15) A gas has a volume of 2 liters at 323 K and 3 atmospheres. When its temperature is changed to 273 K and the pressure is changed to 1 atmosphere, the new volume of the gas would be equal to A) 2 L x 323K/273K x 1atm/3atm B) 2 L x 273K/323K x 1atm/3atm C) 2 L x 323K/273K x 3atm/1atm D) 2 L x 273K/323K x 3atm/1atm
B
15) A solution will boil at the highest temperature when it contains 1 mole of nonvolatile solute dissolved in A) 750 g of solvent B) 250 g of solvent C) 500 g of solvent D) 1,000 g of solvent
C
15) The heat of vaporization for water is 2,260 joules per gram. What is the minimum number of joules needed to change 40.00 grams of water at 100*C to steam at the same temperature and pressure? A) 2,260 B) 40.00 C) 90,400 D) 226,000
C
15) What general type of chemical reaction is illustrated in the particle diagram below? A) decomposition B) double replacement C) single replacement D) synthesis
A
16) As the atmospheric pressure increases, the temperature at which water in an open container will boil A) increases B) remains the same C) decreases
A
16) Given the unbalanced equation: __Al2(SO4)3 + __Ca(OH)2 -> __Al(OH)3 + __CaSO4 When the equation is completely balanced using the smallest whole-number coefficients, the sum of the coefficients is A) 9 B) 3 C) 4 D) 5
B
16) If the pressure and Kelvin temperature of 2.00 moles of an ideal gas at STP are doubled, the resulting volume will be A) 5.60 L B) 44.8 L C) 22.4 L D) 11.2 L
A
16) When 2.00 moles of sugar (C6H12O6) are dissolved in 1.000. grams of water, the boiling point of the resulting solution is closest to A) 101*C B) 100.*C C) 99.5*C D) 99.0*C
D
17) A 20.-milliliter sample of a gas is at 546 K and has a pressure of 6.0 atmospheres. If the temperature is changed to 273 K and the pressure to 2.0 atmospheres, the new volume of the gas will be A) 13 mL B) 3.3 mL C) 120 mL D) 30. mL
B
17) Which equation best describes the reaction shown in the diagram? A) 2AB + C -> A2C + B2 B) A + 2BC -> AB2 + C2 C) A + BC -> AC + B D) A + B2C2 -> AB2 + 2C
B
17) Which sample of water has the greatest vapor pressure? A) 100 mL at 20*C B) 40 mL at 35*C C) 200 mL at 25*C D) 20 mL at 30*C
C
17) Which solution would have the lowest freezing point? A) 0.5 mole of NaCl dissolved in 1,000 g of water B) 1 mole of NaCl dissolved in 1,000 g of water C) 1 mole of NaCl dissolved in 500 g of water D) 0.5 mole of NaCl dissolved in 500 g of water
A
18) A sealed flask contains 1 mole of hydrogen and 3 moles of helium gas at 20*C. If the total pressure is 40 kPa, what is the partial pressure of the hydrogen gas? A) 10 kPa B) 30 kPa C) 40 kPa D) 20 kPa
C
18) What general type of reaction is illustrated in the diagram? A) double replacement B) decomposition C) single replacement D) synthesis
A
18) What is the first phase change that is most likely to occur as the pressure on nitrogen gas is increased and its temperature is decreased? A) condensation B) evaporation C) crystallization D) solidification
A
18) Why is salt (NaCl) put on icy roads and sidewalks in the winter? A) It is ionic and lowers the freezing point of water. B) It is covalent and lowers the freezing point of water. C) It is covalent and raises the freezing point of water. D) It is ionic and raises the freezing point of water.
C
19) A 300.-milliliter container that is filled with 100. milliliters of oxygen and 200. milliliters of hydrogen has a total pressure of 90.0 kPa. What is the partial pressure of the oxygen? A) 200. kPa B) 60.0 kPa C) 30.0 kPa D) 100. kPa
D
19) How do the freezing and boiling points of a sample of water change when 1 mole of NaCl is dissolved in it? A) The freezing point increases and the boiling point increases. B) The freezing point increases and the boiling point decreases. C) The freezing point decreases and the boiling point decreases. D) The freezing point decreases and the boiling point increases.
D
19) The vapor pressure of ethanol at its normal boiling point is A) 100 kPa B) 273 kPa C) 80 kPa D) 101.3 kPa
A
19) When the equation H2 S + O2 -> H2O + SO2 is completely balanced using smallest whole numbers, the sum of all the coefficients is A) 9 B) 7 C) 11 D) 5
A
2) According to the Activity Series chemistry reference table, which pair of substances would undergo a single replacement reaction? A) Li and RbCl B) Rb and LiCl C) Cs and RbCl D) Cs and LiCl
B
2) An assumption of the kinetic theory of gases is that the particles of a gas have A) little attraction for each other and a significant volume B) little attraction for each other and an insignificant volume C) strong attraction for each other and an insignificant volume D) strong attraction for each other and a significant volume
C
2) Given the reaction: N2(g) + 3H2(g) -> 2NH3(g) What is the ratio of moles of H2(g) consumed to moles of NH3(g) produced? A) 6:6 B) 2:3 C) 3:2 D) 1:2
D
2) Ionic solids will most likely dissolve in A) CCl4(l), which is a nonpolar solvent B) CCl4(l), which is a polar solvent C) H2O(l), which is a nonpolar solvent D) H2O(l), which is a polar solvent
B
2) Which mass contains 6.0 x 10^23 atoms? A) 16 g of sulfur B) 28 g of silicon C) 3.0 g of helium D) 6.0 g of carbon
B
2) Which particle diagram best represents a substance in the liquid state? A) A B) B C) C D) D
C
20) How many moles of dissolved particles are required to lower the freezing point of 1,000 grams of water by 5.58 C*? A) 1 B) 2 C) 3 D) 4
A
20) When the equation __C8H16 + __O2 -> __CO2 + __H2O is correctly balanced using the smallest whole number coefficients, the coefficient of O2 is A) 12 B) 16 C) 1 D) 8
D
20) Which change of phase is exothermic? A) liquid to a gas B) solid to a liquid C) solid to a gas D) gas to a liquid
A
20) Which of the following statements correctly compares the number of molecules in the containers? A) All three containers have the same number of molecules. B) Container B has the greatest number of molecules. C) Container C has the greatest number of molecules. D) Container A has the greatest number of molecules.
C
21) Which change results in a release of energy? A) the melting of H2O(s) B) the evaporation of H2O(l) C) the condensation of H2O(g) D) the boiling of H2O(l)
B
21) Which sample of methane gas contains the greatest number of molecules at standard temperature? A) 11.2 liters at 2 atmospheres B) 22.4 liters at 2 atmospheres C) 11.2 liters at 1 atmosphere D) 22.4 liters at 1 atmosphere
C
22) A 1.0 liter flask contains 5.0 moles of a gas at 27.0*C. What is the pressure of the gas? [R = .082 L*atm/mol*k] A) 101.3 atm B) 0.41 atm C) 123 atm D) 300 atm
B
22) The graph below represents the uniform cooling of water at 1 atmosphere, starting with water as a gas above its boiling point. What segments of the cooling curve represent the fixed points on a thermometer? A) CD and EF B) BC and DE C) AB and CD D) AB and EF
B
23) How many moles of gas occupy 22.4 liters at 27*C and 0.50 atm of pressure? [R = .082 L*atm/mol*k] A) 0.25 B) 0.45 C) 2.2 D) 10.0
C
23) The graph below represents the uniform cooling of a substance starting as a gas at 160*C. At which temperature does a phase change occur for this substance? A) 140*C B) 0*C C) 40*C D) 80*C
C
24) A 0.50 mole sample of CO2(g) at 2.0 atm occupies 11.2 liters. What is the temperature of the sample? [R = .082 L*atm/mol*k] A) 273 K B) 546*C C) 546 K D) 273*C
A
24) A student collected data in an experiment in which the uniform cooling of a water sample was observed from 50*C to -32*C. Which graph most likely represents the results obtained by the student? A) A B) B C) C D) D
D
25) The diagram below represents the uniform heating of a water sample at standard pressure, starting at a temperature below 0*C. If 5 grams of water undergoes a temperature change from C to D, the total energy absorbed is A) 418 joules B) 100 joules C) 333.6 joules D) 2,090 joules
D
25) Under the same conditions of temperature and pressure, which noble gas diffuses most rapidly? A) Ar B) Kr C) Xe D) Ne
C
3) A change in pressure would have the greatest effect on the solubility of a A) solid in a liquid B) liquid in a solid C) gas in a liquid D) liquid in a liquid
D
3) A flask containing molecules of gas A and a separate flask containing the molecules of gas B are both at the same temperature. Gases A and B must have equal A) masses B) pressures C) volumes D) average kinetic energies
A
3) Given the reaction: 4Na + O2 -> 2Na2O How many grams of oxygen are completely consumed in the production of 1.00 mole of Na2O? A) 16.0 g B) 124 g C) 62.0 g D) 32.0 g
D
3) Given the unbalanced equation: Li + N2 -> Li3N When the equation is correctly balanced using smallest whole numbers, the coefficient of the lithium is A) 1 B) 2 C) 3 D) 6
A
3) In an equation, what symbol would indicate a gas? A) (g) B) (l) C) (s) D) (aq)
A
3) The total number of sodium atoms in 46.0 grams of sodium is A) 12.0 x 10^23 B) 3.01 x 10^23 C) 24.0 x 10^23 D) 6.02 x 10^23
A
7) At STP, 32.0 liters of O2 contains the same number of molecules as A) 32.0 liters of H2 B) 44.8 liters of He C) 22.4 liters of Ar D) 28.0 liters of N2
D
7) Given the reaction: 2NaOH + H2SO4 -> Na2SO4 + 2H2O What is the total number of grams of NaOH needed to react completely with 196 grams of H2SO4? A) 80 g B) 20 g C) 392 g D) 160 g
B
7) The particles in a crystalline solid are arranged A) regularly and far apart B) regularly and close together C) randomly and far apart D) randomly and close together
A
7) What is the molarity of a solution that contains 112 grams of KOH in 2.00 liters of solution? A) 1.00 M B) 2.00 M C) 3.00 M D) 4.00 M
D
7) When the equation H2 + N2 -> NH3 is completely balanced using the smallest whole numbers, the sum of all the coefficients will be A) 12 B) 7 C) 3 D) 6
D
7) Which graph best shows the change in the volume of 1 mole of nitrogen gas as pressure increases and temperature remains constant? A) A B) B C) C D) D
B
What general type of reaction is illustrated in the diagram? A) double replacement B) synthesis C) single replacement D) decomposition
C
1) According to the kinetic theory of gases, which assumption is correct? A) Gas particles strongly attract each other. B) The volume of gas particles prevents random motion. C) Energy may be transferred between colliding particles. D) Gas particles travel in curved paths.
D
1) Given the reaction: 2KClO3(s) -> 2KCl(s) + 3O2(g) What is the total number of moles of KClO3(s) needed to produce 6 moles of O2(g)? A) 1 B) 2 C) 3 D) 4
C
1) The particle diagrams below represent elements at STP. Which particle diagram best represents helium? A) A B) B C) C D) D
C
1) What is the total mass of oxygen, in grams, in 1.00 mole of Al2 (CrO4)3? A) 64.0 g B) 48.0 g C) 192 g D) 112 g
A
1) Which of the following statements describes KCl(aq)? A) KCl is the solute in a homogeneous mixture. B) KCl is the solvent in a homogeneous mixture. C) KCl is the solute in a heterogeneous mixture. D) KCl is the solvent in a heterogeneous mixture.
B
4) A 1-gram sample of which substance in a sealed 1-liter container will occupy the container completely and uniformly? A) Hg(l) B) H2O(g) C) Ag(s) D) H2O(l)
D
4) Given the reaction: 3Cu + 8HNO3 -> 3Cu(NO3)2 + 2NO + 4H2O The total number of grams of Cu needed to produce 1.0 mole of Cu(NO3)2 is A) 128 g B) 32 g C) 192 g D) 64 g
A
4) One reason that a real gas deviates from an ideal gas is that the molecules of the real gas have A) forces of attraction for each other B) no net loss of energy on collision C) a straight-line motion D) a negligible volume
D
4) What is the total number of atoms contained in 2.00 moles of nickel? A) 118 B) 6.02 x 10^23 C) 58.9 D) 1.20 x 10^24
D
4) Which balanced chemical equation represents a synthesis reaction? A) MgBr2(l) -> Mg(l) + Br2(g) B) C2H4(g) + 3O2(g) -> 2CO2(g) + 2H2O(g) C) Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g) D) 2Al(s) + 3Cl2(g) -> 2AlCl3(s)
C
4)Which graph most closely represents the data shown in the table? A) A B) B C) C D) D
B
5) Given the balanced equation: NaOH + HCl -> NaCl + H2O What is the total number of grams of H2O produced when 116 grams of the product, NaCl, is formed? A) 9.0 g B) 36 g C) 54 g D) 18 g
A
5) Given the unbalanced equation: __C3H8(g) + __O2(g) -> __H2O(g) + __CO2(g) When the equation is completely balanced using smallest whole numbers, the coefficient of O2 A) 5 B) 2 C) 3 D) 10
A
5) Under what conditions does a real gas behave most like an ideal gas? A) at high temperatures and low pressures B) at low temperatures and high pressures C) at high temperatures and high pressures D) at low temperatures and low pressures
D
5) Which gas sample contains a total of 3.0 x 10^23 molecules? A) 2.0 g of H2 B) 71 g of Cl2 C) 38 g of F2 D) 14 g of N2
D
5) Which set of properties does a substance such as CO2(g) have? A) no definite shape but definite volume B) definite shape and definite volume C) definite shape but no definite volume D) no definite shape and no definite volume
B
5) Which solution is the most concentrated? A) 0.3 mole of solute dissolved in 200 mL of solvent B) 0.4 mole of solute dissolved in 100 mL of solvent C) 0.1 mole of solute dissolved in 400 mL of solvent D) 0.2 mole of solute dissolved in 300 mL of solvent
B
6) As the pressure of a gas at 101.3 kPa is changed to 50.65 kPa at constant temperature, the volume of the gas A) remains the same B) increases C) decreases
D
6) Given the equation: Zn + 2HCl -> ZnCl2 + H2 How many grams of HCl would be required to produce a total of 4.0 grams of H2? A) 18 g B) 36 g C) 288 g D) 144 g
B
6) The chemical reaction Zn(s) + CuSO4(aq) -> ZnSO4(aq) + Cu(s) is best described as a A) synthesis reaction B) single replacement reaction C) double replacement reaction D) combustion reaction
D
6) Under the same conditions of temperature and pressure, a liquid differs from a gas because the particles of the liquid A) are in constant straight-line motion B) have no regular arrangement C) take the shape of the container they occupy D) have stronger forces of attraction between them
B
6) Which sample of neon contains a total of 3.01 x 10^23 molecules at STP? A) 20.0 g B) 11.2 L C) 40.0 g D) 22.4 L
D
6) Which solution contains the greatest number of moles of solute? A) 0.5 L of 2 M B) 0.5 L of 0.5 M C) 2 L of 0.5 M D) 2 L of 2 M
C
8) A 100. milliliter sample of a gas at a pressure of 50.65 kPa is reduced to 25.33 kPa at constant temperature. What is the new volume of the gas? A) 290. mL B) 50.0 mL C) 200. mL D) 90.0 mL
C
8) Given the reaction: 2CO + O2 -> 2CO2 What is the minimum number of grams of CO required to produce 88 grams of CO2? A) 88 g B) 28 g C) 56 g D) 64 g
A
8) How many grams of KOH are needed to prepare 250. milliliters of a 2.00 M solution of KOH (formula mass = 56.0)? A) 28.0 g B) 2.00 g C) 1.00 g D) 112 g
D
8) The characteristic which distinguishes a true solid from other phases of matter at STP is that in a true solid, the particles are A) vibrating and changing their relative positions B) motionless but changing their relative positions C) motionless without changing their relative positions D) vibrating without changing their relative positions
D
8) What is the percent by mass of oxygen in Ca(OH)2? A) 74 B) 16 C) 22 D) 43
C
8) When C3H8 burns completely in an excess of oxygen, the products formed are A) CO and H2O B) CO and H2 C) CO2 and H2O D) CO2 and H2
D
9) Given the balanced equation: 2Na + 2H2O -> 2X + H2 What is the correct formula for the product represented by the letter X? A) NaO B) Na2O C) Na2OH D) NaOH
A
9) Given the reaction: Ca(s) + 2H2O(l) -> Ca(OH)2(aq) + H2(g) When 40.1 grams of Ca(s) reacts completely with the water, what is the total volume, at STP, of H2(g) produced? A) 22.4 L B) 2.00 L C) 1.00 L D) 44.8 L
A
9) The number of joules per gram required to melt ice at its melting point is called A) heat of fusion B) sublimation C) heat of vaporization D) vapor pressure
B
9) The percent by mass of nitrogen in Mg(CN)2 is equal to A) 14/76 x 100 B) 28/76 x 100 C) 28/50 x 100 D) 14/50 x 100
D
9) The volume of a given mass of an ideal gas at constant pressure is A) inversely proportional to the Celsius temperature B) inversely proportional to the Kelvin temperature C) directly proportional to the Celsius temperature D) directly proportional to the Kelvin temperature
B
9) What is the total number of grams of KCl (formula mass = 74.6) in 1.00 liter of 0.200 molar solution? A) 29.8 g B) 14.9 g C) 7.46 g D) 22.4 g
B
Given the reaction: 4NH3(g) + 5O2(g) -> 4NO(g) + 6H2O(g) 10) What is the total number of liters of O2(g) required to produce 40 liters of NO? A) 5.0 L B) 50. L C) 32 L D) 9.0 L
A
Given the reaction: 4NH3(g) + 5O2(g) -> 4NO(g) + 6H2O(g) 11) At STP, what is the total volume of O2(g) required to produce 80.0 liters of NO(g)? A) 100. L B) 5.00 L C) 80.0 L D) 20.0 L
